Chapter Four: Chemical Bonds and Compounds Overview

Chemical Bond

Attraction holding atoms in a compound.

Ionic Bond

Electrons transferred, forming oppositely charged ions.

Covalent Bond

Atoms share electrons to form bonds.

Chemical Formula

Simplest representation of a molecule.

Empirical Formula

Lowest whole number ratio of atoms.

Molecular Formula

Exact number of atoms in a molecule.

Structural Formula

Shows atom arrangement and bond types.

Atomic Element

Element consisting of single atoms.

Molecular Element

Element with multiple atoms of the same type.

Molecular Compound

Composed solely of nonmetals.

Ionic Compound

Contains cations and anions.

Diatomic Element

Element existing as two atoms bonded together.

Lewis Symbols

Representation of valence electrons using dots.

Octet Rule

Atoms gain, lose, or share electrons for eight.

Naming Ionic Compounds

Cation name first, then anion name.

Type I Cation

Cation with a fixed charge.

Type II Cation

Cation with variable charge indicated in parentheses.

Polyatomic Ion

Ion consisting of multiple atoms.

Hydrate

Ionic compound with water molecules attached.

Single Covalent Bond

Two atoms share one pair of electrons.

Double Covalent Bond

Two atoms share two pairs of electrons.

Triple Covalent Bond

Two atoms share three pairs of electrons.

Naming Molecular Compounds

Use prefixes to denote number of atoms.

Acid

Compound with H+ ion attached to anion.

Oxyacid

Acid with oxygen in its anion.

Molecular Mass

Mass of one mole of a compound.

Percent Composition

Mass percentage of each element in a compound.

Empirical vs Molecular Formula

Empirical shows ratio; molecular shows exact count.

Combustion Analysis

Determines empirical formula from combustion products.